The first ionization energy is the energy that is required in order to remove the first electron from an atom in the GAS phase, the second ionization energy is the energy required to remove the second electron from an atom, etc. Ionization energy generally increases for every electron that is removed, and increases from left to right in the Periodic Table or if moving up the periods.
In this case, from the periodic table (or according to Mastering Chemistry) Bromine (Br) has a larger sixth ionization energy than Selenium (Se).
Se should have a larger ionization energy than Br. This is because Se, located in the higher period on the periodic table, has a larger atomic radius compared to Br. As you move across a period from left to right, the ionization energy generally increases due to increased effective nuclear charge.
Bismuth (Bi) has a higher ionization energy than bromine (Br) because bismuth is a larger atom with more electron shells, making it more difficult to remove an electron. Additionally, bismuth is in the p-block of the periodic table, where ionization energies generally increase across a period.
The first ionization energy of bromine is approximately 1139 kJ/mol. This is the energy required to remove one electron from a bromine atom in the gas phase to form a Br+ ion.
The ionization energy of an element is influenced by its atomic structure and the ease with which electrons can be removed. Bromine (Br) has a higher ionization energy than chlorine (Cl) because it is located further away from the nucleus, resulting in less shielding and higher attraction for its outermost electron. Selenium (Se) has a lower ionization energy than bromine because it is in a higher energy level, making its outermost electron easier to remove.
Bromine (Br) is more reactive than chlorine (Cl) and selenium (Se). Bromine has a lower ionization energy and a larger atomic radius compared to chlorine and selenium, making it more willing to participate in chemical reactions.
Se should have a larger ionization energy than Br. This is because Se, located in the higher period on the periodic table, has a larger atomic radius compared to Br. As you move across a period from left to right, the ionization energy generally increases due to increased effective nuclear charge.
Bismuth (Bi) has a higher ionization energy than bromine (Br) because bismuth is a larger atom with more electron shells, making it more difficult to remove an electron. Additionally, bismuth is in the p-block of the periodic table, where ionization energies generally increase across a period.
Krypton has a higher value.
The first ionization energy of bromine is approximately 1139 kJ/mol. This is the energy required to remove one electron from a bromine atom in the gas phase to form a Br+ ion.
The ionization energy of an element is influenced by its atomic structure and the ease with which electrons can be removed. Bromine (Br) has a higher ionization energy than chlorine (Cl) because it is located further away from the nucleus, resulting in less shielding and higher attraction for its outermost electron. Selenium (Se) has a lower ionization energy than bromine because it is in a higher energy level, making its outermost electron easier to remove.
Bromine (Br) is more reactive than chlorine (Cl) and selenium (Se). Bromine has a lower ionization energy and a larger atomic radius compared to chlorine and selenium, making it more willing to participate in chemical reactions.
HCl (aq) + H2O (L) ---------> H3O+ (aq) + Cl- (aq)
The Br ion is larger than the K ion. This is because the Br ion has more electron shells than the K ion, leading to a larger atomic radius.
No. The Se ion will be larger than the Br ion. The more negative the anion's charge, the larger the radius (more electrons = stronger repulsion between the electrons; so, more distance between them). Se would become "Se2-" as an anion, and Br would become "Br1-". Because Se's "2-" anion charge is more negative than Br's "1-" anion charge, and because Se would have more relative electrons to protons than Br, there is more repulsion between electrons, and distance, within the Se ion. So, the Se ion has a larger radius. Hope it helps.
Na has a larger atomic radius than Br. This is because Na is a metal and atoms in metals have larger atomic radii compared to nonmetals like Br, which has a smaller atomic radius due to its higher effective nuclear charge.
The bond between Br-I is more polar than the bond between Br-Cl. This is because iodine is less electronegative than chlorine, resulting in a larger difference in electronegativity between the two atoms in the bond. Therefore, the Br-I bond will exhibit stronger polarity.
Calcium has atomic number 20 and bromine is 35, so bromine has a bigger nucleus if that is what you mean